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Unit 3: Bonding
Term | Definition |
---|---|
Electron configuration | The arrangement of electrons in an atom. |
Covalent bond | A bond formed when atoms share one or more pairs of electrons. |
ionic bond | A force that attracts electrons fro one atom to another, which transforms a neutral atom into ion. |
ion | an atom, radical, or molecule that has gained or lost one or more electrons and has negative or positive charge. |
Lewis dot structure (electron-dot notation) | A structural formula in which electrons are represented by dots. |
Octet rule | an atom will be most stable when surrounded by 8 electrons in the valence shell (outer most energy level) |
metallic bond | A bond formed by the attraction between positively charged metal ions and the electrons around them. |
conductivity | Material that is able to conduct electricity |
polar | Describes a molecule in which the positive and negative charges are separated. |
nonpolar | A covalent bond in which the bonding electrons are equally attracted to both bonded atoms. |
bent | 2,2 |
tetrahedral | 4,0 |
trigonal planar | 3,0 |
linar | 2,0 |
valence electrons | An electron that is found in the outermost shell of an atom and that determines the atom's chemical properties. |
formula unit | The simplest collection of atoms from which an ionic compound's formula can be written. |
polyatomic ion | A covalent bonded set of two or more atoms, or of a metal complex, that can be considered to behave as a single unit and that has a net charge that is not zero. |
VSEPR theory | A theory that predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other. |